1) Molar composition
Base: 100 g
C: 40.00 g / 12.0 g /mol = 3.333 mol
H: 6.72 g / 1 g/mol = 6.72 mol
O: 53.28 g / 16g/mol = 3.33 mol
2) Divide by the smaller number of moles
C: 3.333 / 3.33 = 1.00
H: 6.72 / 3.33 = 2.02 ≈ 2
O: 3.33/3.33 = 1.00
3) Empirical formula
CH2O
molar mass of the empirical formula = 12 g/mol + 2*1g/mol + 16 g/mol = 30 g/,ol
4) Number of times that the mass of empirical formula is contained in the molar mass = 180 g/mol / 30 g/mol = 6
5) Molecular formula = 6 times the empirical formula
=>C6H12O6
Answer: C6H12O6
I found this information:
Anaerobic respiration begins the same way as fermentation. The first step is still glycolysis, and it still creates 2 ATP from one carbohydrate molecule. However, instead of ending with glycolysis, as fermentation does, anaerobic respiration creates pyruvate and then continues on the same path as aerobic respiration.
After making a molecule called acetyl coenzyme A, it continues to the citric acid cycle. More electron carriers are made and then everything ends up at the electron transport chain. The electron carriers deposit the electrons at the beginning of the chain and then, through a process called chemiosmosis, produce many ATP. For the electron transport chain to continue working, there must be a final electron acceptor. If that acceptor is oxygen, the process is considered aerobic respiration.
Scientists believe that fermentation and anaerobic respiration are older processes than aerobic respiration.
I hope this help. :)
have a good day!
Molarity is a concentration unit, the number of moles of solute divided by the numbers of liters in a solution. Pertaining to chem
Answer: When one thing in a <u>electric</u> circuit stops working, the whole circuit stops working.
Explanation:
Explanation:
For what I can see, is missing the concentration of [Ag+] in the half-cell. To calculate it:
Niquel half-cell
Oxidation reaction: 
![E=E^0 - \frac{R*T}{n*F}*ln(1/[Ni^{2+}])](https://tex.z-dn.net/?f=E%3DE%5E0%20-%20%5Cfrac%7BR%2AT%7D%7Bn%2AF%7D%2Aln%281%2F%5BNi%5E%7B2%2B%7D%5D%29)
Assuming T=298 K / R=8.314 J/mol K / F=96500 C
Silver half-cell
Reduction reaction: 
![E=E^0 - \frac{R*T}{n*F}*ln(1/[Ag+])](https://tex.z-dn.net/?f=E%3DE%5E0%20-%20%5Cfrac%7BR%2AT%7D%7Bn%2AF%7D%2Aln%281%2F%5BAg%2B%5D%29)
Assuming T=298 K / R=8.314 J/mol K / F=96500 C
![0.835V=0.8V - \frac{8.314*298}{1*96500}*ln(1/[Ag+])](https://tex.z-dn.net/?f=0.835V%3D0.8V%20-%20%5Cfrac%7B8.314%2A298%7D%7B1%2A96500%7D%2Aln%281%2F%5BAg%2B%5D%29)
![[Ag+]=0.26 M](https://tex.z-dn.net/?f=%5BAg%2B%5D%3D0.26%20M)
